Nuclear Chemistry
1. Given the mass defect for the triton (tritium nucleus) to be 0.00910 amu, calculate the binding
energy per nucleon: 1 amu = 931.4 MeV.
a) 2.119 MeV
b) 2.825 MeV
c) 4.238 MeV
d) 8.476 MeV
2. If an unstable nucleus decays by successive alpha, beta, beta emissions, the overall change in
the atomic number and the mass number are respectively
a) —4 and 0
b) +2 and —2
c) 0 and —4
d) —2 and —4
3. What is the binding energy per nucleon for 17O? The masses of the electron, proton, and
neutron are 0.000549 amu 1.007276 amu and 1.008665 amu, respectively. The atomic mass of
17O is 16.99903 amu. The speed of light is 2.9979 × 1010 cm/sec.
1 erg = 1 g-cm2/sec2.
a) 1.24 × 10—5 erg/nucleon
b) 1.32 × 10—5 erg/nucleon
c) 2.11 × 10—4 erg/nucleon
d) 7.48 × 1018 erg/nucleon
4. Iodine-131 has a half-life of 8.1 days and is used as a tracer for the thyroid gland. If a patient
drinks a sodium iodide (NaI) solution containing iodine-131 on a Tuesday, how many days will it
take for the concentration of iodine-131 to drop to 5.0% of its initial concentration?
a. 19 days
b. 35 days
c. 0.81 day
d. 4.3 days
e. 8.1 days
5. Nuclear fission produces energy because __________
a. neutrons are produced.
b. the total mass of the products is less than that of the reactants.
c. the total mass of the products is more than that of the reactants.
d. it is a very powerful chemical reaction.
e. photons are produced.
6. Uranium-235 is the fuel in nuclear power plants. When a nucleus of uranium-235 captures a
neutron, the nucleus splits into two lighter nuclei and initiates a chain reaction. The chain
reaction is driven by the emission of __________
a. protons
b. β particles. c. neutrons.
d. α particles. e. positrons
238
𝐴
4
7. In the nuclear equation 92𝑈 → 𝑍𝑋 + 2𝐻𝑒, the letters Z and A are, respectively
(A) 90 and 234
(B) 90 and 242
(C) 94 and 234
(D) 94 and 242
8. The isotope least likely to be found in the band of stability among the following is _____.
a.
C.
c.
Al.
b.
O.
d.
Si.
9. During electron capture, a proton in the nucleus of an atom is converted into a(n) _____.
a.
neutron.
c.
electron.
b.
positron.
d.
another proton.
10. When a nuclide undergoes beta-decay
a) the mass number remains unchanged and the atomic number increases by one
b) the atomic number remains unchanged and the mass number increases by one
c) the mass number remains unchanged and the atomic number decreases by one
d) the atomic number remains unchanged and the mass number decreases by one
Air Chemistry
1. The density of CO gas at 1.00 atm and 323K is 1.06 g/L. What is the density of NO gas at the
same temperature and pressure?
a) 0.989 g/L
b) 1.06 g/L
c) 1.14 g/L
d) 22.4 g/L
2. All of the following are a consequence of Charles’s law EXCEPT
a) A balloon filled with hot air will rise.
b) If the absolute temperature of an ideal gas is doubled, its volume will double as long as the
pressure remains constant.
c) Increasing the pressure on a gas will decrease its volume.
d) An ideal gas would have a volume of 0 L at 0 K regardless of the pressure.
3. Water reacts with lithium to produce H2 gas and LiOH. This reaction is run at 27°C and a pressure
of 0.75 atm. What is the mass of the lithium sample if 3.4 L of H2 are produced using an excess
of HCl?
a) 0.36 g
b) 0.72 g
c) 3.99 g
d) 7.98
4. A gas mixture of N2(g) and CO2(g) contained in a volume of 10.0 L has a total pressure of 0.750
atm at a temperature of 273K. The mixture is known to contain 3.00 g N2(g). What is the partial
pressure of CO2(g) in the mixture?
a) 0.120 atm b) 0.240 atm c) 0.510 atm d) 0.630 atm
5. A flask of 0.5 L volume contains one atmosphere of nitrogen gas at 295K temperature. A vacuum
pump exhausts the flask to a pressure of 1 × 10—7 atm. About how many molecules of nitrogen
remain in the flask?
a) 2.5 × 1012 molecules b) 1.25 × 1015 molecules c) 2.5 × 1019 molecules d) 1.25 × 1022 molecules
General Chemistry
1. A sample of an iron oxide weighing 14.8 g is heated in a stream of H2(g) until it is completely
converted to iron. If the iron produced weighs 10.36 g, the percentage of oxygen in the original
oxide must have been:
a) 14.3%
b) 30.0%
c) 70.0%
d) 85.7%
2. Temporary hardness is due to the presence of
a. calcium carbonate
b. calcium bicarbonate
c. magnesium sulphate
d. calcium sulphate
3. Tincture iodine is a solution of
a. iodine in potassium iodide b. iodine in alcohol
c. iodine in water
d. iodine in carbon disulphide
4. White vitriol is
a. ZnSO4 . 7H2O
b. FeSO4 . 7H2O
c. MgSO4 . 7H2O
d. CaSO4 . 2H2O
5. The average atomic mass of Ga is 69.72. Naturally occurring Ga is composed of 60.0% 69Ga,
which has an atomic mass of 68.91, and 40.0% of 71Ga. What is the atomic mass of 71Ga?
a) 69.72 amu b) 69.92 amu c) 70.94 amu d) 71.00 amu
Electrochemistry
1. What mass of Cu metal will be deposited in the electrolytic refining of metal using a current of
1.5 A for 10 hours? Consider the process to be a 2 electrons reduction, the molecular mass of Cu
to be 63.55 g/mol, and F = 96500 C/mol.
a) 0.28 g
b) 4.4 × 10—3 g
c) 4.4 × 105 g
d) 1.9 × 103 g
2. One of the original octahedral complexes investigated by Alfred Werner, the founder of the field
of coordination chemistry (for which he was given the Nobel Prize for Chemistry in 1913) was
[Pt(NH3)5Cl]Cl3. The oxidation state (or "primary valency" as Werner called it) for platinum in this
coordination complex is
a) +3
b) +4
c) +5
d) +6
3. Consider the following half-cells connected in a spontaneous (galvanic) cell,
Mn2+ + 2e— → Mn —1.18 V
Ni2+ + 2e— → Ni —0.250 V
Which of the following describes the Mn electrode correctly?
a) Anode and positively charged
b) Cathode and positively charged
c) Anode and negatively charged
d) Cathode and negatively charged
4. Consider a cell in which one half-cell has a lead electrode immersed in a 1M Pb2+ solution and
the other has an iron electrode immersed in a 1M Fe3+ solution. Pertinent reduction potentials
are:
Pb2+ + 2e— → Pb
—0.126 V
Fe3+ + 3e— → Fe
—0.037 V
What will be the cell potential if the cell proceeds spontaneously?
a) 0.089 V
b) 0.163 V
c) 0.304 V
d) 0.489 V
5. In the equation for the reaction of potassium iodide (KI) and sulfuric acid (H2SO4), which
statement is TRUE?
8KI(aq) + 9H2SO4(aq) → 4I2(s) + 8KHSO4(aq) + H2S(g) + 4H2O(l)
a) The reducing agent is H2SO4
b) The oxidizing agent is KI
c) The substance reduced is H2SO4
d) The substance oxidized is KHSO4
6. The reduction of aqueous copper (II) with iron metal has a ∆E° value of 0.78 V.
Fe(s) + Cu2+(aq, 1 M) → Fe2+(aq, 1 M) + Cu(s).
If the standard reduction potential for Cu2+ + 2e— → Cu(s) is 0.34 V, then the standard
reduction potential for Fe2+/Fe(s) must be:
a) 0.44 V
b) —0.44 V
c) 0.22 V
d) —0.22 V
7. The following reaction represents the process used to produce iron from iron (III) oxide:
Fe2O3 + 3CO → 2Fe + 3CO2
What is the reducing agent in this process?
A. Fe
B. CO
C. CO2
D. Fe2O3
8. The process used to deposit one metal over another metal is called
a. Electrolysis
b. electroplating
c. carbon plating
d. none of above
9. In a reaction, the oxidation number of Cr decreases by 3. This indicates that Cr is
A. reduced.
B. oxidized.
C. neutralized.
D. a reducing agent.
10. A given amount of electric charge deposits 2.159 g of silver from an Ag+ solution. What mass of
copper from a Cu2+ solution will be deposited by the same quantity of electric charge? Atomic
Molar Masses: Ag 107.9 g/mol; Cu 63.5 g/mol
a) 0.635 g
b) 1.27 g
c) 1.97 g
d) 2.54 g
Thermochemistry
1. A substance with high specific heat:
a. Is a conductor.
b. Is exothermic
c. Metals are typical examples.
d. Requires more energy to raise the temperature than a substance with lower specific heat.
2. The value of ∆H for the following reaction is +52.0 kJ/mol at 298K. What is the
value of ∆U in kJ/mol at the same temperature?
6C(s) + 3H2(g) → C6H6(l)
a) 44.6 kJ/mol b) 52.0 kJ/mol
c) 54.5 kJ/mol d) 59.4 kJ/mol
3. Blocks A and B are made from different metals and have the same mass. When they are heated
with 500 J of energy, block A increases 15°C, while block B increases 90°C. Which has a larger
specific heat?
a. Block A
b. Block B
c. They have the same specific heat.
D. There is not enough information to
compare.
4. What is the enthalpy change of the third reaction in terms of the enthalpy changes of the first
two reactions?
2H2(g) + O2(g)
→ 2H2O(l)
∆H1
4NH3(g) + 3O2(g) → 6H2O(l) + 2N2(g)
∆H2
4NH3(g)
→ 6H2(g) + 2N2(g)
∆H3
a) ∆H3 = ∆H2 — ∆H1/2
b) ∆H3 = ∆H2/2 — 3∆H1
c) ∆H3 = ∆H2 — ∆H1
d) ∆H3 = ∆H2 — 3∆H1
5. 10. g of ice at 0.0°C is dropped into 30. g of liquid water at 80°C. ∆Hfusion of water at 0.0°C is
6.00 kJ/mol. What is the final temperature?
a) 40°C
b) 43°C
c) 46°C
d) More information is required
6. How much energy is required to change the temperature of 2.00 g aluminum from 20.0°C to
25.0°C? The specific heat of aluminum is 0.902 J/g- °C.
a. 2.3 J
b. 9.0 J
c. 0.36 J
d.0.090 J
7. Which one is not a state function
a. Internal energy
b. Enthalpy
c. Gibbs free energy
d. Work
8. Which of the following statements is true?
a) The standard enthalpy of formation of a compound is the enthalpy of the formation of the
compound from the atoms that compose it.
b) The standard enthalpy of formation of a compound is the enthalpy of the formation of the
compound in its standard state from the elements that compose it in their standard states.
c) The standard enthalpy of formation of a compound is always a negative number.
d) The standard enthalpy of formation of an element is zero regardless of what state it is in.
9. We can generate hydrogen chloride by hating a mixture of sulfuric acid and potassium chloride
according to the equations:
2KCl(s) + H2SO4(l) → 2HCl(g) + K2SO4(s)
Calculate H in kJ for this reaction from the following thermochemical equations:
HCl(g) + KOH(s) → KCl(s) + H2O(l)
H = -203.6 kJ
H2SO4(I) +2KOH(s) →K2SO4(s) + 2H2O(l) H = -342.4 kJ
A) 64.8kJ
B) -138.8kJ
C) 138.8 kJ
D) -64.8kJ
10. Enthalpy of a reaction can be measured by
a. Glass calorimeter
b. Manometer
c. Barometer
d. Thermometer
Organic Chemistry
1. When a straight chain alkene undergoes sulfuric acid catalyzed hydration, the primary product is
a __________.
a) primary alcohol
b) secondary alcohol c) tertiary alcohol
d) quaternary alcohol
2. When compound X was added to a dilute solution of potassium permanganate at room
temperature, the solution immediately turned from purple to a murky brown color. Which one
of the following compounds could compound X be?
a) methane
b) ethylene
c) propane
d) 5-chlorodecane
3. Oxidation of which of the following compounds can lead to an aldehyde?
a) A primary alcohol b) A secondary alcohol
c) A tertiary alcohol
d) An ether
4. Hydrolysis of an ester leads to two compounds. Which of the following pairs compounds is
formed from such a hydrolysis?
a) An alcohol and an aldehyde
b) Two alcohols
c) An alcohol and a carboxylic acid
d) A ketone and a carboxylic acid
5. Which of the following compounds would you expect to be the most soluble in water?
a) CH3CH2CH2CH2CH2CH2CH2CH3
b) CH3CH2CH2OH
c) CH3CH2CH2CH2CH2CH2CH2OH
d) CH3CH2CH2-O-CH2CH2CH3
6. The reaction of methane with chlorine to form methyl chloride follows a free radical chain
reaction mechanism. The first step in this reaction mechanism is __________________.
a) abstraction of a hydrogen from a methane molecule by a chlorine molecule
b) homolytic splitting of the chlorine molecule into chlorine atoms
c) photochemical splitting of one of the C-H bonds in methane
d) reaction of a hydrogen from methane with a chlorine molecule to form HCl which then
catalyzes the reaction
7. When benzene reacts with chlorine, a(n) ____ reaction occurs whereas when cyclohexene
reacts with chlorine a(n) ____ reaction occurs.
a) oxidation, reduction
b) addition, oxidation
c) substitution, oxidation
d) substitution, addition
8. Which compound is not a constitutional isomer of but-2-ene, CH3CH=CHCH3?
a.
9.
10.
11.
12.
13.
14.
15.
c.
b.
d.
Ether functional group can be represented as
a. ROH
b. R-CO-R
c. R-O-R
d. R-COOH
Give the IUPAC name of this compound: CH3OCH2CH3.
a. dimethyl ether
b. methoxyethane
c. methylethyloxide
d. propyl ether
All of the following are true about alkynes EXCEPT
a) They contain one or more carbon-carbon triple bonds.
b) They have the general formula CnH2n.
c) They contain at least two sp hybridized carbons.
d) The simplest one, acetylene, can be made by the reaction of water and calcium carbide.
Which of the following react most readily with Br2?
a) Straight chain alkanes
b) Branched alkanes c) Alkenes
d) Aromatic compounds
Which of the following compounds does NOT undergo mutarotation?
a. glucose
b. sucrose
c. ribose
d. fructose
Which acid is described as H00CCOOH
a. Carbonic acid
b. Oxalic acid
c. Acetic acid
d. Formic acid
Which compound has the highest melting point?
a. decane
b. 2,2,3,3-tetramethylbutane
c. 2,2,3-trimethylpentane
d. 4-methylnonane